Sodium persulfate
Sodium persulfate | |
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Other names Sodium peroxodisulfate | |
Identifiers | |
CAS number | 7775-27-1 |
PubChem | 62655 |
ChemSpider | 56406 |
EC number | 231-892-1 |
UN number | 1505 |
ChEMBL | CHEMBL502764 |
RTECS number | SE0525000 |
Jmol-3D images | {{#if:[Na+].[Na+].O=S(=O)([O-])OOS([O-])(=O)=O|Image 1 |
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Properties | |
Molecular formula | Na2S2O8 |
Molar mass | 238.10 g/mol (19.31& Na, 53.76% O, 26.93% S) [1] |
Appearance | white powder |
Density | 2.40 g/cm3
Loose bulk density = 1.12 g/cm3[2] Crystal density = 2.59 g/cm3[3] |
Melting point | 180 °C decomp. |
Solubility in water | 55.6 g/100 ml (20 °C) |
Hazards | |
MSDS | ICSC 1136 |
EU Index | Not listed |
R-phrases | R8 R20 R22 R36 R37 R38 |
S-phrases | S17 S26 S36 |
NFPA 704 |
0
2
1
OX
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Flash point | Non-flammable |
Related compounds | |
Other anions | Sodium dithionite Sodium sulfite Sodium sulfate |
Other cations | Potassium persulfate |
(verify) (what is: / ?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa) | |
Infobox references | |
Sodium persulfate (Na2S2O8) is a chemical compound. It is a strong oxidizer. It is a severe irritant of the skin, eyes, and respiratory system. It is almost non-hygroscopic and has particularly good ability to be stored for long time. It is easy and safe to handle. It is not combustible, but releases oxygen easily and assists combustion of other materials.
It is used as a bleach, both standalone (particularly in hair cosmetics) and as a detergent component. It is a replacement for ammonium persulfate in etching mixtures for zinc and printed circuit boards, and is used for pickling of copper and some other metals. It is a source of free radicals, making it useful as a radical initiator for emulsion polymerization reactions and for accelerated curing of low formaldehyde adhesives. It is also used as a soil conditioner and in manufacture of dyestuffs, modification of starch, bleach activator, desizing agent for oxidative desizing, etc.
Conditions/substances to avoid mixing persulfates with are: moisture, heat, flame, ignition sources, shock, friction, reducing agents, organic material, sodium peroxide, water, aluminium, and powdered metals.
Sodium persulfate is an oxidizing agent in chemistry, for example in a synthesis of diapocynin from apocynin where iron(II) sulfate is the radical initiator:[4]
Sodium persulfate is synthesized using water and sodium sulfate (Na2SO4 * 10H2O) in electrolysis with a pure platinum anode. [5] ( Link to IR Spectra [6] )
The standard redox potential of sodium persulfate into hydrogen sulfate is 2.1 V, which is higher than that of hydrogen peroxide (1.8 V) but lower than ozone (2.2 V).[7] The sulfate radical formed in situ has a standard electrode potential of 2.7 V.
References
- ↑ Anonymous Sodium Persulfate. In Merck Index; O'Neil, M. J., Ed.; Merck & Co., Inc.: Whitehouse Station, NJ, 2006; pp 1488.
- ↑ FMC Corporation. Sodium Persulfate. http://www.fmcchemicals.com/Portals/chem/Content/docs/Tech%20Data%20Sheets/sodpersulfate.pdf (accessed Nov 17, 2013).
- ↑ FMC Corporation. Sodium Persulfate. http://www.fmcchemicals.com/Portals/chem/Content/docs/Tech%20Data%20Sheets/sodpersulfate.pdf (accessed Nov 17, 2013).
- ↑ Luchtefeld, Ron; Dasari, Mina S.; Richards, Kristy M.; Alt, Mikaela L.; Crawford, Clark F. P.; Schleiden, Amanda; Ingram, Jai; Hamidou, Abdel Aziz Amadou et al. (2008). "Synthesis of Diapocynin". J. Chem. Ed. 85 (3): 411. doi:10.1021/ed085p411.
- ↑ Pietzsch, A.; Adolph, G. J. Chem. Technol. Biotechnol. 1911, 30, 85.
- ↑ Anonymous. Spectral Database for Organic Compounds. http://sdbs.db.aist.go.jp/sdbs/cgi-bin/direct_frame_disp.cgi?sdbsno=40242 (accessed Oct 7, 2013).
- ↑ Block, Philip A., Richard A. Brown, and David Robinson. "Novel activation technologies for sodium persulfate in situ chemical oxidation." Proceedings of the Fourth International Conference on the remediation of chlorinated and recalcitrant compounds. 2004.
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